Half a mole of an ideal monoatomic gas is heated at a constant pressure of $1\, atm$ from $20\,^oC$ to $90\,^oC$. The work done by the gas is close to ..... $J$ (Gas constant $R = 8.31\, J/mol\cdot K$).

$A$ diatomic gas $(\gamma = 1.4)$ does $200 \,J$ of work when it is expanded isobarically. The heat given to the gas in the process is: (in $\,J$)

The ratio of specific heats of a gas is $\gamma$. The change in internal energy of one mole of the gas, when the volume changes from $V$ to $2V$ at constant pressure $p$, is:

$A$ monoatomic gas is supplied heat $Q$ very slowly keeping the pressure constant. The work done by the gas will be

The temperature of $1$ mole of an ideal monoatomic gas is increased by $50^{\circ} C$ at constant pressure. The total heat added and change in internal energy are $E_1$ and $E_2$,respectively. If $\frac{E_1}{E_2}=\frac{x}{9}$,then the value of $x$ is . . . . . . .

In an isobaric process,